Question

How do you write an ionic equation for the following reaction? a student repeats the experiments with copper instead of magnesium. state whether a reaction would still occur. Why or why not?

Answer 1

An understudy rehashes the investigation with copper rather than magnesium. $Mg\left( s \right) + F{e_2} + \left( {aq} \right) \to M{g_2} + \left( {aq} \right) + Fe\left( s \right)$; No response if $Cu\left( s \right)$is utilized instead of $Mg\left( s \right)$. They are to counteract in the net ionic condition the manner in which one would drop.

Complete step by step answer:
Similar to a subatomic condition, which communicates mixes as particles, an ionic condition is a synthetic condition wherein the electrolytes in aqueous arrangement are communicated as separated particles. Furthermore, the net charge is the equivalent on the two sides of the condition. The particles in aqueous arrangements are settled by particle dipole interactions with water atoms. In any case, an ionic condition might be composed for any electrolyte that separates and responds in a polar dissolvable. In a fair ionic condition, the number and sort of molecules are the equivalent on the two sides of the response bolt. Moreover, the net charge is the equivalent on the two sides of the condition. Solid acids, solid bases, and dissolvable ionic mixes (normally salts) exist as separated particles in aqueous arrangement, so they are composed as particles in the ionic condition. Powerless acids and bases and insoluble salts are generally composed utilizing their sub-atomic equations on the grounds that a limited quantity of them separates into particles. There are exemptions, particularly with corrosive base responses. Regardless of whether such a response happens can be dictated by In the event that the principles express that a particle is dissolvable, at that point it stays in its aqueous particle structure. antigens; be that as it may, the climate where this happens is as yet being considered.

Note:
An ionic condition is a compound condition where the electrolytes in aqueous arrangement are composed as separated particles.